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Element Folio

Category: Elements & Periodic Table

Element profiles, periodic trends, groups and periodic-table reference guides.

  • Helium (He): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Helium (He) has atomic number 2 and is classified as a noble gas. It sits in Group 18, period 1 of the periodic table. Its practical relevance includes cryogenic cooling, leak detection, inert atmospheres and scientific instrumentation.

    Quick facts

    Atomic number 2 Symbol He
    Relative atomic mass 4.0026 State at room temperature Gas
    Group 18 Period 1
    Classification noble gas Block s-block

    Position in the periodic table

    Noble gases have filled valence shells and are relatively unreactive under ordinary conditions. Their inertness is valuable in lighting, welding, semiconductor processing, cryogenics and scientific instrumentation.

    Helium belongs to period 1. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Helium matters

    In engineering and technology, helium is associated with cryogenic cooling, leak detection, inert atmospheres and scientific instrumentation. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of helium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Helium depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Neon (Ne) · Argon (Ar) · Krypton (Kr) · Hydrogen (H)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Beryllium (Be): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Beryllium (Be) has atomic number 4 and is classified as a alkaline earth metal. It sits in Group 2, period 2 of the periodic table. Its practical relevance includes aerospace structures, X-ray windows, precision components and copper-beryllium alloys.

    Quick facts

    Atomic number 4 Symbol Be
    Relative atomic mass 9.0122 State at room temperature Solid
    Group 2 Period 2
    Classification alkaline earth metal Block s-block

    Position in the periodic table

    Alkaline earth metals are reactive s-block metals that commonly form +2 ions. Their compounds are important in construction, refractories, metallurgy, chemicals and biological systems.

    Beryllium belongs to period 2. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Beryllium matters

    In engineering and technology, beryllium is associated with aerospace structures, X-ray windows, precision components and copper-beryllium alloys. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of beryllium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Beryllium depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Magnesium (Mg) · Calcium (Ca) · Strontium (Sr) · Lithium (Li)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Boron (B): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Boron (B) has atomic number 5 and is classified as a metalloid. It sits in Group 13, period 2 of the periodic table. Its practical relevance includes borosilicate glass, boron carbide, detergents, nuclear control materials and semiconductor doping.

    Quick facts

    Atomic number 5 Symbol B
    Relative atomic mass 10.81 State at room temperature Solid
    Group 13 Period 2
    Classification metalloid Block p-block

    Position in the periodic table

    Metalloids sit near the boundary between metals and nonmetals. Their intermediate electrical and chemical behavior makes several of them especially important in semiconductors, glass, ceramics and electronic materials.

    Boron belongs to period 2. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Boron matters

    In engineering and technology, boron is associated with borosilicate glass, boron carbide, detergents, nuclear control materials and semiconductor doping. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of boron depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Boron depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Aluminum (Al) · Gallium (Ga) · Indium (In) · Beryllium (Be)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Nitrogen (N): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Nitrogen (N) has atomic number 7 and is classified as a nonmetal. It sits in Group 15, period 2 of the periodic table. Its practical relevance includes fertilizer production, inerting, food preservation, cryogenics and chemical processing.

    Quick facts

    Atomic number 7 Symbol N
    Relative atomic mass 14.007 State at room temperature Gas
    Group 15 Period 2
    Classification nonmetal Block p-block

    Position in the periodic table

    Nonmetals show very different bonding and physical behavior from metals. They are essential to chemistry, energy, biological systems and many modern materials, often appearing as gases, molecular solids or network structures.

    Nitrogen belongs to period 2. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Nitrogen matters

    In engineering and technology, nitrogen is associated with fertilizer production, inerting, food preservation, cryogenics and chemical processing. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of nitrogen depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Nitrogen depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Phosphorus (P) · Arsenic (As) · Antimony (Sb) · Carbon (C)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Fluorine (F): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Fluorine (F) has atomic number 9 and is classified as a halogen. It sits in Group 17, period 2 of the periodic table. Its practical relevance includes fluoropolymers, uranium processing, specialty chemicals, pharmaceuticals and semiconductor manufacturing.

    Quick facts

    Atomic number 9 Symbol F
    Relative atomic mass 18.998 State at room temperature Gas
    Group 17 Period 2
    Classification halogen Block p-block

    Position in the periodic table

    Halogens are reactive p-block elements that commonly form -1 ions and many important salts or organic compounds. Their industrial value is substantial, but elemental forms and some compounds can require strict corrosion, toxicity or containment controls.

    Fluorine belongs to period 2. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Fluorine matters

    In engineering and technology, fluorine is associated with fluoropolymers, uranium processing, specialty chemicals, pharmaceuticals and semiconductor manufacturing. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of fluorine depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Fluorine depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Chlorine (Cl) · Bromine (Br) · Iodine (I) · Oxygen (O)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Neon (Ne): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Neon (Ne) has atomic number 10 and is classified as a noble gas. It sits in Group 18, period 2 of the periodic table. Its practical relevance includes sign lighting, indicator lamps, lasers and specialized cryogenic research.

    Quick facts

    Atomic number 10 Symbol Ne
    Relative atomic mass 20.180 State at room temperature Gas
    Group 18 Period 2
    Classification noble gas Block p-block

    Position in the periodic table

    Noble gases have filled valence shells and are relatively unreactive under ordinary conditions. Their inertness is valuable in lighting, welding, semiconductor processing, cryogenics and scientific instrumentation.

    Neon belongs to period 2. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Neon matters

    In engineering and technology, neon is associated with sign lighting, indicator lamps, lasers and specialized cryogenic research. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of neon depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Neon depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Helium (He) · Argon (Ar) · Krypton (Kr) · Fluorine (F)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Sodium (Na): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Sodium (Na) has atomic number 11 and is classified as a alkali metal. It sits in Group 1, period 3 of the periodic table. Its practical relevance includes bulk chemicals, sodium-vapor lighting, heat-transfer systems and metal refining.

    Quick facts

    Atomic number 11 Symbol Na
    Relative atomic mass 22.990 State at room temperature Solid
    Group 1 Period 3
    Classification alkali metal Block s-block

    Position in the periodic table

    Alkali metals are highly reactive s-block metals with one valence electron. Their chemistry is dominated by +1 oxidation states, and they require careful handling because several react vigorously with air or water.

    Sodium belongs to period 3. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Sodium matters

    In engineering and technology, sodium is associated with bulk chemicals, sodium-vapor lighting, heat-transfer systems and metal refining. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of sodium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Sodium depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Hydrogen (H) · Lithium (Li) · Potassium (K) · Neon (Ne)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Magnesium (Mg): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Magnesium (Mg) has atomic number 12 and is classified as a alkaline earth metal. It sits in Group 2, period 3 of the periodic table. Its practical relevance includes lightweight alloys, desulfurization, refractories, pyrotechnics and sacrificial anodes.

    Quick facts

    Atomic number 12 Symbol Mg
    Relative atomic mass 24.305 State at room temperature Solid
    Group 2 Period 3
    Classification alkaline earth metal Block s-block

    Position in the periodic table

    Alkaline earth metals are reactive s-block metals that commonly form +2 ions. Their compounds are important in construction, refractories, metallurgy, chemicals and biological systems.

    Magnesium belongs to period 3. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Magnesium matters

    In engineering and technology, magnesium is associated with lightweight alloys, desulfurization, refractories, pyrotechnics and sacrificial anodes. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of magnesium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Magnesium depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Beryllium (Be) · Calcium (Ca) · Strontium (Sr) · Sodium (Na)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Aluminum (Al): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Aluminum (Al) has atomic number 13 and is classified as a post-transition metal. It sits in Group 13, period 3 of the periodic table. Its practical relevance includes transport, construction, packaging, electrical conductors and aerospace structures.

    Quick facts

    Atomic number 13 Symbol Al
    Relative atomic mass 26.982 State at room temperature Solid
    Group 13 Period 3
    Classification post-transition metal Block p-block

    Position in the periodic table

    Post-transition metals lie mainly in the p-block and often combine metallic conductivity with comparatively low melting points or distinctive alloying behavior. Their applications span electronics, solders, coatings and specialized process materials.

    Aluminum belongs to period 3. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Aluminum matters

    In engineering and technology, aluminum is associated with transport, construction, packaging, electrical conductors and aerospace structures. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of aluminum depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Aluminum depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Boron (B) · Gallium (Ga) · Indium (In) · Magnesium (Mg)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Phosphorus (P): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Phosphorus (P) has atomic number 15 and is classified as a nonmetal. It sits in Group 15, period 3 of the periodic table. Its practical relevance includes fertilizers, specialty chemicals, metallurgy, flame retardants and semiconductor processing.

    Quick facts

    Atomic number 15 Symbol P
    Relative atomic mass 30.974 State at room temperature Solid
    Group 15 Period 3
    Classification nonmetal Block p-block

    Position in the periodic table

    Nonmetals show very different bonding and physical behavior from metals. They are essential to chemistry, energy, biological systems and many modern materials, often appearing as gases, molecular solids or network structures.

    Phosphorus belongs to period 3. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Phosphorus matters

    In engineering and technology, phosphorus is associated with fertilizers, specialty chemicals, metallurgy, flame retardants and semiconductor processing. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of phosphorus depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Phosphorus depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Nitrogen (N) · Arsenic (As) · Antimony (Sb) · Silicon (Si)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons